Dichlorine hexoxide is the chemical compound with the molecular formula , which is correct for its gaseous state. However, in liquid or solid form, this chlorine oxide ionizes into the dark red ionic compound chloryl perchlorate , which may be thought of as the mixed Acidic oxide, anhydride of chloric acid, chloric and perchloric acids. It is produced by reaction between chlorine dioxide and excess ozone: :2 + 2 → 2 + 2 → + 2

Molecular structure

It was originally reported to exist as the monomeric chlorine trioxide ClO₃ in gas phase, but was later shown to remain an oxygen-bridged dimer after evaporation and until thermal decomposition into chlorine perchlorate, Cl₂O₄, and oxygen. The compound ClO₃ was then rediscovered. It is a dark red fuming liquid at room temperature that crystallizes as a red ionic compound, chloryl perchlorate, . The red color shows the presence of chloryl ions. Thus, chlorine's formal oxidation state in this compound remains a mixture of chlorine (V) and chlorine (VII) both in the gas phase and when condensed; however by breaking one oxygen-chlorine bond some electron density does shifts towards the chlorine (VII).

Properties

Cl₂O₆ is diamagnetic and is a very strong oxidizing agent. Although stable at room temperature, it explodes violently on contact with organic compounds and reacts with gold to produce the chloryl salt . Many other reactions involving Cl₂O₆ reflect its ionic structure, , including the following: :NO₂F + Cl₂O₆ → NO₂ClO₄ + ClO₂F :NO + Cl₂O₆ → NOClO₄ + ClO₂ :2 V₂O₅ + 12 Cl₂O₆ → 4 VO(ClO₄)₃ + 12 ClO₂ + 3 O₂ :SnCl₄ + 6 Cl₂O₆ → [ClO₂]₂[Sn(ClO₄)₆] + 4 ClO₂ + 2 Cl₂ :2Au + 6Cl₂O₆ → 2 + Cl₂ Nevertheless, it can also react as a source of the ClO₃ radical: :2 AsF₅ + Cl₂O₆ → 2 ClO₃AsF₅

References

{{oxygen compounds Chlorine oxides Acidic oxides Perchlorates Chloryl compounds Chlorine(V) compounds Chlorine(VII) compounds